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Question
A dilute ferrous sulphate solution is gradually added to the beaker containing acidified permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation?
Options
KMnO4 is an oxidising agent and it oxidises FeSO4
FeSO4 acts as an oxidising agent and it oxidises KMnO4
The colour disappears due to dilution; no reaction is involved
KMnO4 is an unstable compound and decomposes in presence of FeSO4 to a colourless compound.
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Solution
KMnO4 is an oxidising agent and it oxidises FeSO4
Explanation -
Potassium permanganate (KMnO4) is an oxidising agent. It oxidises ferrous sulphate to ferric sulphate in the presence of dilute
H2SO4.
`underset("Purple")(2"KMnO"_4) + 8"H"_2"SO"_4 + 10"FeSO"_4 -> "K"_2"SO"_4 + 2"MnSO"_4 + 8"H"_2"O" + 5"Fe"_2("SO"_4)_3`
By taking part in the reaction, the light purple colour of the solution slowly fades and finally disappears.
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